Iodine is a non metal element. Atomic mass number of it is 127.
Smaller
The empirically measured covalent radius of tin is 145 pm; for iodine this radius is 140 pm.
Fr (Francium) has the largest atomic size compared to Li (Lithium) because Francium is located at the bottom of group 1 on the periodic table, which means it has more energy levels and electron shells compared to Lithium, hence larger atomic size.
Iodine reacts slowest with iron compared to other halogens such as fluorine, chlorine, and bromine because iodine's lower reactivity due to its larger atomic size and weaker electronegativity.
In rubidium, having a larger atomic radius, the attraction force between the atomic nucleus and and the electron from outermost shell is lower.
Rubidium has a larger atomic radius than sodium because rubidium has more electrons and energy levels, leading to increased electron-electron repulsion and a larger atomic size. Additionally, the outermost electron in rubidium is in a higher energy level compared to sodium, contributing to a larger atomic radius.
Cesium has a larger atomic radius than rubidium. This is because as you move down a group in the periodic table, the atomic radius generally increases due to the addition of more energy levels and electrons.
The atomic radius of iodine is larger than the atomic radius of potassium. This is because as you move down a group in the periodic table, atomic size increases due to the addition of more electron shells. Iodine is located below potassium in the periodic table, hence it has a larger atomic radius.
Rubidium is the least reactive, followed by potassium, and then lithium. This trend is due to the increase in reactivity as you move down the alkali metal group on the periodic table, with larger atoms having more easily discarded outer electrons, making them more reactive.
Rubidium is softer than potassium. This is because rubidium has larger atomic size and higher reactivity, which makes it more easily deformable when compared to potassium.
Iodine is a non metal element. Atomic mass number of it is 127.
Smaller
The lattice energy of potassium bromide is more exothermic than that of rubidium iodide because potassium and bromine have smaller atomic sizes and higher charges, which leads to stronger ionic bonding in potassium bromide. Rubidium and iodine have larger atomic sizes and lower charges, resulting in weaker ionic bonding in rubidium iodide. The stronger ionic bonding in potassium bromide requires more energy to break, resulting in a more exothermic lattice energy.
Rubidium is more reactive than sodium because rubidium has a larger atomic radius and fewer electron shells, making it easier for rubidium to lose an electron and form a positive ion. This tendency to lose an electron increases its reactivity compared to sodium.
K has a larger atomic radius than Li. This is because atomic radius generally increases down a group in the periodic table, so potassium (K) being below lithium (Li) in Group 1 will have a larger atomic radius.
The atomic radius of Sr (Strontium) is larger than that of Rb (Rubidium). This is because atomic radius generally increases down a group in the periodic table, and Sr is located below Rb in the same group.